Lithium carbonate (Li2CO3) is not very soluble in water (0.13 mg/mL), whereas po

Question

Lithium carbonate (Li2CO3) is not very soluble in water (0.13 mg/mL), whereas potassium carbonate (K2CO3) is more soluble in water (11 mg/mL). See the PEC diagrams-> Ep Ep 2 K(aq) co(aq) Li,Co,(s) H2o(l) 2 Li(aq) co(aq) K,CO3(s) # of configurations # of configurations Explain how increasing temperature would affect the solubility of the two compounds above. 1. 2. Comment on whether the ion-ion forces (ionic interactions) are stronger than the ion-dipole forces (hydration interactions) for Li2COs and K2COs, when each is dissolved in water Explain why Li2COs is less soluble than K2CO3. Mention physical differences between Li and K, and how that affects the number of configurations when each ion is dissolved in water 3.

Explanation / Answer

1.With the increase in temperature the solubility of both increases but there is always Li2CO3 less soluble due smaller size and easy to form covalent bond with CO3-.

2.ion ion forces are more stronger than ion dipole forces

3.Li+ being smaller in size can form the easy covalent bond with the CO3- so unable to dissociate to form interactions with water molecules.

Li+ is has more covalent nature than K+.

Li+ has small size than K+

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